Course title:
Chemistry
Course Description:
Students will study chemistry using problem solving skills and through performing experiments. Throughout the course students will investigate the relationship between matter and energy. Students will investigate principles of chemistry using scientific method, analysis, and practical application. Areas of study will include chemistry concepts, terminology, lab experimentation, data collection, history and current issues related to chemical principles.
Course Prerequisites:
Successful completion of high school science class , Geometry and Algebra 1
Major Objectives or Topics:
Lessons are categorized under the topic headers: air, water, earth, water, prime and void. Major topics include, but are not limited to: periodic table, molecular structure, reactions, and states of matter.
Materials:
Computer, internet access and lab supplies
Assignment Overview:
Objective assignments
Writing assignments
Labs
Viruses Project
End of Course Test
Grading Procedures:
Each lesson will be graded based upon skill mastery. Students will be asked to revise work until it meets the minimum requirements outlined by the grading rubric on each lesson.
Submission Policy: Students are to complete course lessons in orders. Each day a student may post either two new lessons, or 2 revisions, or a lesson and a revision in each course. Unless permission to work on more than two lessons has been granted by the teacher, students should only work on two lessons at a time. Once a lesson is graded, students may move on to the next lesson
Communication: Students may communicate with their teacher using the Teachermail. On the Student Desk, students will find links to Guidance, Technical Help, and Transcripts.
Lessons:
Air
Lesson 1 - Basic Elements
Lesson 2 - Terminology and Symbols for Elements
Lesson 3 - Nuclear Radiation
Lesson 4 - Shells And Orbitals
Lesson 5 - Review
Water
Lesson 6 - Terminology and Symbols for Molecules
Lesson 7 - Covalent Bonds and Lewis Structures
Lesson 8 - Ionic and Metal Bonds
Lesson 9 - Weak Bonds and Physical Properties
Lesson 10 - Shapes of Molecules
Earth
Lesson 11 - Typical Elements
Lesson 12 - Periodic Table: Properties of the Elements
Lesson 13 - Periodic Table: Overview of the Elements
Lesson 14 - Review
Fire
Lesson 15 - Chemical Reactions
Lesson 16 - Reactions: Balancing Equations
Lesson 17 - Reactions: Rate and Equilibrium
Prime
Lesson 18 - The Mole, Mass, and Reactions
Lesson 19 - Stoichiometric Calculations
Lesson 20 - Solutions
Lesson 21 - Phases of Matter
Void
Lesson 22 - Organic Chemistry
Chemistry Objectives by Lesson
Lesson 1: Basic Elements VA SOL: CH.1, CH.2
Learning Objectives:
§ Students learn about the basic structure of atoms and their subatomic particles.
§ Students learn the characteristics of subatomic particles and how there are related to an atom’s mass and charge.
§ Students learn about the most abundant atoms in the universe and how all the known atoms were originally created.
§ Students learn the definition and significance of an atom’s atomic number and are introduced to the concept of isotopes and natural abundance.
§ Students are introduced to transmutation, beta decay, and radiation.
§ Students learn about atomic mass, Daltons, and the difference between mass and weight.
§ Students are introduced to the periodic table.
Lesson 2: Terminology and Symbols for Elements VA SOL: CH.1, CH.2
Learning Objectives:
§ Students learn elemental and isotopic symbols.
§ Students are introduced to writing chemical and nuclear equations.
§ Students relate the atomic number and mass number to the number of subatomic particles in any isotope.
Lesson 3: Nuclear Radiation VA SOL: CH.1, CH.2
Learning Objectives:
§ Students learn the history of the discovery of radiation and nuclear chemistry.
§ Students learn about alpha, beta, and gamma radiation (most common forms of radiation): their similarities and differences and their effect on the atoms that produce them as well as their relative energies and damage potential.
§ Students learn the concept of half-life and how to calculate the amount of a radioactive isotope remaining given half-life information.
§ Students learn that half-life is isotope specific, that most naturally-occurring isotopes are not radioactive, and how radioactivity is measured.
§ Students are introduced to the concept that the nucleus is held together by strong nuclear forces.
§ Students complete specific activity calculations and are first introduced to the unit conversion methods.
§ Students are introduced to the Big Bang theory and how it relates to nuclear fusion and fission reactions and the creation of the majority of the elements.
§ Students are asked to investigate a science-based societal issue
Lesson 4: Shells and Orbitals VA SOL: CH.1, CH.2
Learning Objectives:
§ Students learn how to determine the number of electron in an atom from the atomic number.
§ Students learn that the atomic size is determined by the position of the outermost electrons.
§ Students determine the number of electrons that atoms have available for bonding.
§ Students are introduced to the concept of electrons occupying shells of different energy around the nucleus.
§ Students are introduced to the basic consequences of quantum mechanics (without specifics).
§ Students learn about the maximum electron occupancy of the first four shells and their orbitals.
§ Students learn about orbitals and their shapes and geometries.
§ Students learn the proper method of orbital electron filling in neutral atoms
Lesson 5 Review
Lesson 6: Terminology and Symbols for Molecules VA SOL: CH.1, CH.3
Learning Objectives:
§ Students learn to identify compound and elemental molecules and to calculate their molecular mass.
§ Students learn how to write molecular formulas.
§ Students are introduced to the concept of bonding and the role electrons play in bonding
Lesson 7: Covalent Bonds and Lewis Structures VA SOL: CH.1, CH.3
Learning Objectives:
§ Students are introduced to Bohr and Lewis and the modern concept of atomic and molecular structure.
§ Students learn that chemical reactions occur between outer shell e- of adjacent atoms.
§ Students learn different bonding types.
§ Students learn to construct Lewis dot structures.
§ Students learn that chemical bonds are between atoms can share one, two, or three electrons pairs, to form single, double, or triple bonds
§ Students learn about the noble gases and why they are inert.
Lesson 8: Ionic and Metal Bonds VA SOL: CH.1, CH.3
Learning Objectives:
§ Students learn how ions and ionic bonds are formed.
§ Students learn to identify cations and anions.
§ Students are introduced to electrostatic forces and how they relate to bonding.
§ Students predict the charges certain atoms will likely make when becoming ions.
§ Students are introduced to electronegativity.
§ Students learn to construct ionic compound formulas from their atoms.
§ Students learn the similarities and differences between covalent, ionic, and metallic bonds.
Lesson 9: Weak Bonds and Physical Properties VA SOL: CH.1
Learning Objectives:
§ Students are introduced to intermolecular forces and the differences in strength between IMF’s and intramolecular bonding.
§ Students learn to use electronegativity to determine bond polarity.
§ Students learn about molecular polarity and how that influences IMF strength and solubility.
§ Students are introduced to solvation spheres in aqueous solution and saturated solutions.
§ Definitions and examples of Van der Waals forces and hydrogen bonding are identified, and their relative strengths are explained.
§ Students learn the link between IMF’s and physical properties, including the four states of matter.
§ Students are introduced to the concept of energy as it relates to phase changes, and temperature as it relates to molecular motion, IMF’s, and states of matter.
Lesson 10 - Shapes of Molecules VA SOL: CH.1
Learning Objectives:
§ Students learn to use Lewis structures to determine geometries of simple molecules.
§ Molecular and hybrid orbitals are introduced in a rudimentary way to describe covalent bonding and then related to molecular geometry.
§ VSEPR theory is explained and used to determine molecular shapes of simple molecules.
§ Students learn to recognize shape in three dimensions.
§ Students learn about hybridization of orbitals.
§ Students learn to relative repulsive force of bonding and non-bonding electron pairs and how this influences molecular shapes.
§ Shapes of ionic and metallic molecules are also discussed.
Lesson 11 - Periodic Table: Typical Elements VA SOL: CH.1, CH.2
Learning Objectives:
§ Students are introduced to the history of the development of the periodic table.
§ Students learn to relate the position of elements in the periodic table to atomic number, atomic mass and electron configuration.
§ Students learn of trends in ion formation and chemical properties in relation to place on the periodic table.
§ Students learn nomenclature of monatomic ionic compounds.
Lesson 12 - Periodic Table: Properties of the Elements
Learning Objectives:
§ Students learn the relationship between periodicity and properties such as atomic radius, electron affinity, ionization energy, and electronegativity.
§ Students are introduced to the metric system.
§ Students examine the allotropic forms of carbon.
§ Students characterize covalent and ionic bond character and how these relate to polarity of bonds and molecules.
Lesson 13 - Periodic Table: Overview of the Elements
Learning Objectives:
§ Students present descriptive chemistry information on the first ten elements.
§ Students categorize elements as metals, non-metals, and semi-metals, and learn their positions on the periodic table.
§ Students learn the names and chemical properties of the Group A elements.
§ Students are given an overview of the transition metals as well as the actinides and lanthanides.
Lesson 14 - Review
Lesson 15 - Chemical Reactions VA SOL: CH.1, CH.3
Learning Objectives:
§ Students describe chemical reactions by writing balanced equations and identifying different types of reactions.
§ Students are introduced to exothermic and endothermic reactions.
§ Students learn nomenclature of covalent compounds.
Lesson 16 - Balancing Equations VA SOL: CH.1, CH.3
Learning Objectives:
§ Students learn the names and formulas of common polyatomic ions the nomenclature associated with compounds containing them.
§ Students learn naming rules for transition metal compounds.
§ Students develop equation balancing techniques.
Lesson 17 - Reaction Rate and Equilibrium VA SOL: CH.1, CH.3
Learning Objectives:
§ Students learn to recognize the rate of reaction as it relates to the concentrations of reactants and products.
§ Students learn the factors affecting reaction rates.
§ Students define and learn examples of activation energy.
§ Students examine the function of catalysts.
§ Students learn the definition of dynamic equilibrium and how to write equilibrium constant expressions from balanced equilibrium equations.
§ Students examine LeChatlier’s Principle.
Lesson 18 - The Mole, Conservation of Mass and Chemical Reactions VA SOL: CH.1, CH.4
Learning Objectives:
§ Students determine the molar mass of atoms and compounds.
§ Students learn why the mole concept is useful and that 1 mole has 6.02 x 1023 particles.
§ Students learn to complete basic stoichiometric calculations.
Lesson 19 - Stoichiometric Calculations VA SOL: CH.1, CH.4
Learning Objectives:
§ Students complete mole/mole, mass/mole, and mass/mass stoichiometry.
§ Students find mass of reactants and products in chemical reactions from the mass of a given reactant or product.
§ Students calculate percent yield of a chemical reaction.
§ Students calculate the amount of products based upon a limiting reagent, as well as determining the limiting reagent and calculating the amount of excess reagent remaining after the reaction is complete.
§ Students learn that mass is conserved in chemical reactions.
§ Unit conversions are required throughout these lessons.
Lesson 20 – Solutions VA SOL: CH.1, CH.4
Learning Objectives:
§ Students learn the definitions of solute, solvent, and solution, and learn different types of solutions.
§ Students learn the factors that affect the dissolving process.
§ Students determine the concentration of a solute in a solution, with a focus on molarity.
§ Students interpret a solubility graph.
§ Students examine the relationship of concentration to solution properties.
§ Students learn the symbols associated with different phases as written in chemical reactions, including equilibrium reactions.
§ Strong, weak, and non-electrolyte solutions are defined and identified.
§ Colligative properties such as boiling point elevation and freezing point depression are introduced.
Lesson 21 – Phases of Matter VA SOL: CH.1, CH.5
Learning Objectives:
§ Students learn that random motion of molecules and their collisions with a surface create the pressure on that surface.
§ Students learn the definition and value of standard temperature and pressure and absolute zero.
§ Students must convert between Kelvin and Celsius temperature scales.
§ Students apply Graham’s Law and understand the concept of effusion.
§ Students learn and apply – both qualitatively and quantitatively – the gas laws, both in static and changing conditions.
§ Students relate the temperature of a gas to its average kinetic energy, and analyze chemical processes in terms of heat.
§ Students learn the basics of the phases of matter
§ Students learn the basics of the kinetic-molecular theory of gases.
§ Students learn the difference between ideal and non-ideal gases
§ Students recognize properties of vapor pressure
§ Students identify causes of phase changes
Lesson 22 – Organic Chemistry VA SOL: CH.1, CH.6
Learning Objectives:
Students learn to identify organic molecules and their different functional groups.
Lewis structures are used to illustrate the variety of covalent bonds that carbon can form.
Students learn that repeating combinations of simple sub-units are linked to form large organic molecules.
Students learn that amino acids are the building blocks of proteins.
Students investigate household polymers and identify their monomers.
Course Course Outcomes
Outcome Descriptionrelate the position of elements in the periodic table to their atomic number and atomic mass
recognize metals, semimetals, and nonmetals by their position on the periodic table
describe and interpret the trends in properties of elements
determine the number of electrons atoms have available for bonding
illustrate that the mass of an atom depends on the number of protons and neutrons in the nucleus, while atomic size is determined by the position of the outermost electrons